A chemist must dilute of aqueous iron (II) bromide solution until the concentration falls to. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits.

Question

Dorsey

Chemistry

2 July, 10:24

A chemist must dilute of aqueous iron (II) bromide solution until the concentration falls to. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits.

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Answers (1)

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Ashly Hendricks · Answer 1

22.9 mL

Explanation:

use dilution formula

M1*V1 = M2*V2

1---> is for stock solution

2---> is for diluted solution

Assuming the values not given in the question

M1 = 2.41 M

M2 = 2.0 M

V1 = 19.0 mL

Use:

M1*V1 = M2*V2

V2 = (M1*V1) / M2

V2 = (2.41*19) / 2

V2 = 22.9 mL

22.9 mL